Chemistry

Lecture 1 : Importance of Chemistry ; Nature of Matter ; Significant figures ; Empirical and molecular formula

Lecture 2 : Chemical reactions ; Uncertainty in Measurement ; Laws of Chemical Combinations

Lecture 3 : Dalton’s Atomic Theory ; Atomic and Molecular Masses ; Mole concept and molar masses and percentage composition ; Stochiometry and stoichiometric calculation

Lecture 4: Revison

Lecture 1: Sub-atomic Particles: Discovery of electrons ; Discovery of protons and neutrons ; Charge to mass ratio of electrons ; Miliken’s oil drop experiment

Lecture 2: Atomic Models: Thomsons model of atom ; Rutherfords’ model and limitation ; Atomic number and mass number, isotopes and isobars ; Bohr’s model

Lecture 3:Wave nature of electromagnetic radiation ; Plank’s quantum theory ; Photoelectric effect ; Atomic spectra

Lecture 4:Line spectrum of Hydrogen ; Bohr’s Model for Hydrogen Atom ; Towards Quantum-Mechanical Model of the Atom ; Dual behavior of matter

Lecture 5: Heisenberg Uncertainty Principle ; Quantum Mechanical Model of Atom ; Hydrogen atom and Schrodinger equation ; Orbitals and quantum number

Lecture 6: Shapes of atomic orbital ; Energy of atomic orbitals ; Auf Bau’s principle, Pauli’s exclusion principle, Hund’s rule of maximum multiplicity ; Electronic configuration of atoms, stability of completely filled and half filled electrons

Lecture 7: Revison

Lecture 1: Why do we need to classify elements ; Genesis of periodic classification ; Modern periodic law and the present form of periodic table

Lecture 2: Nomenclature of elements having atomic atoms > 100 ; Electronic configuration of elements and the periodic table ; Electronic configuration and type of elements: s,p,d, and f blocks

Lecture 3: Metal non-metals and metalloids ; Ionic radius ; Ionisation enthalpy

Lecture 4: Electron gain enthalpy ; Electronegativity

Lecture 5: Valency or oxidation states ; Anamolous property of second group elements ; Periodic trend and chemical reactivity

Lecture 6: Revison

Lecture 1: Kossel-Lewis approach to chemical bonding D.2 Octet rule ; Octet rule ; Covalent bonding ; Lewis representation of simple molecules

Lecture 2 : Formal charge ; Limitation to octet rule ; Bond parameters ; Resonance structures

Lecture 3 : Polarity of bonds ; VSEPR theory ; Shapes of simple molecules according to VSEPR theory ; Valence bond theory

Lecture 4 : Orbital overlap concept ; Type of orbital overlap ; Hybridisation ; Types of hybridization involving sp,sp2, sp3 and sp3d

Lecture 5 : Molecular orbital theory ; Linear combination of atomic orbitals (LCAO) ; Condition for combination of atomic orbitals ; Bonding in some homonuclear diatomic molecules; Hydrogen bonding

Lecture 6: Revison

Lecture 1: Intermolecular forces ; Intermolecular forces vs thermal interactions ; The gaseous state

Lecture 2: Boyle’s law ; Charle’s law ; Gay Lussac law

Lecture 3 : Ideal gas equation ; Dalton’s law of partial pressure ; Kinetic molecular theory of gases

Lecture 4 : Behaviour of real gas: Deviation from ideal gas ; Liquifaction of gas ; Liquid state- vapor pressure ; Viscosity and surface tension

Lecture 5: Revison

Chapter 6 - Thermodynamics

Chapter 7 - Equilibrium

Chapter 8 - Redox Reactions

Chapter 9 - Hydrogen

Chapter 10 - The s-Block Elements

Chapter 11 - The p-Block Elements

Chapter 12 - Organic Chemistry – Some Basic Principles and Techniques

Chapter 13 - Hydrocarbons

Chapter 14 - Environmental Chemistry